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The peak lowers, and the curve flattens. This indicates a wider distribution of speeds, meaning more particles are moving at very high speeds, and fewer are concentrated around the average. 3. POGIL Extension Question: The Effect of Molecular Mass
The Maxwell–Boltzmann distribution | AP Chemistry | Khan Academy The peak lowers, and the curve flattens
This feature is designed to bridge the gap between the standard "reading" of the graph and the "application" required in the extension questions. It provides scaffolding for students to predict how the curve changes before they calculate or graph it, specifically focusing on and Molar Mass . POGIL Extension Question: The Effect of Molecular Mass
Concise sample: common formulas (for teaching/answers) some molecules move much faster
Two gases, ( \textO_2 ) (molar mass 32 g/mol) and ( \textHe ) (molar mass 4 g/mol), are at the same temperature.
Other acceptable answers: Increase concentration (more collisions, but not changing speed distribution) — but question asks for “changing molecular speed distribution,” so temperature is best.
When you add heat to a gas, the average kinetic energy of its molecules increases. With more energy on average, the entire distribution shifts to higher energies. The curve broadens because the increased energy allows for a wider range of molecular speeds; some molecules move much faster, while far fewer move at very low speeds. This shift has critical implications for chemical reactions, as a larger fraction of molecules will now have energy exceeding the activation energy ($E_a$), leading to a higher reaction rate.
The peak lowers, and the curve flattens. This indicates a wider distribution of speeds, meaning more particles are moving at very high speeds, and fewer are concentrated around the average. 3. POGIL Extension Question: The Effect of Molecular Mass
The Maxwell–Boltzmann distribution | AP Chemistry | Khan Academy
This feature is designed to bridge the gap between the standard "reading" of the graph and the "application" required in the extension questions. It provides scaffolding for students to predict how the curve changes before they calculate or graph it, specifically focusing on and Molar Mass .
Concise sample: common formulas (for teaching/answers)
Two gases, ( \textO_2 ) (molar mass 32 g/mol) and ( \textHe ) (molar mass 4 g/mol), are at the same temperature.
Other acceptable answers: Increase concentration (more collisions, but not changing speed distribution) — but question asks for “changing molecular speed distribution,” so temperature is best.
When you add heat to a gas, the average kinetic energy of its molecules increases. With more energy on average, the entire distribution shifts to higher energies. The curve broadens because the increased energy allows for a wider range of molecular speeds; some molecules move much faster, while far fewer move at very low speeds. This shift has critical implications for chemical reactions, as a larger fraction of molecules will now have energy exceeding the activation energy ($E_a$), leading to a higher reaction rate.